Advertisements
Advertisements
Question
Explain whether a gas approaches ideal behavior or deviates from ideal behaviour if the temperature is raised while keeping the volume constant.
Advertisements
Solution
When the temperature is increased, the compressibility factor approaches unity. Hence, the gas behaves ideally.
APPEARS IN
RELATED QUESTIONS
Maximum deviation from ideal gas is expected from
Can a Van der Waals gas with a = 0 be liquefied? explain.
Explain whether a gas approaches ideal behavior or deviates from ideal behaviour if it is compressed to a smaller volume at a constant temperature.
Which of the following gases would you expect to deviate from ideal behavior under conditions of low-temperature F2, Cl2, or Br2? Explain.
If 1 gram of each of the following gases are taken at STP, which of the gases will occupy (a) greatest volume and (b) smallest volume?
\[\ce{CO, H2O, CH4 , NO}\]
Value of universal gas constant (R) is same for all gases. What is its physical significance?
Compressibility factor, Z, of a gas is given as Z = `(pV)/(nRT)`. For real gas what will be the effect on value of Z above Boyle’s temperature?
Match the following graphs of ideal gas with their co-ordinates:
| Graphical representation | x and y co-ordinates |
(i) ![]() |
(a) pV vs. V |
(ii) ![]() |
(b) p vs. V |
(iii) ![]() |
(c) p vs. `1/V` |
Assertion (A): At constant temperature, pV vs V plot for real gases is not a straight line.
Reason (R): At high pressure all gases have \[\ce{Z}\] > 1 but at intermediate pressure most gases have \[\ce{Z}\] < 1.
Choose the correct option for the total pressure (in atm.) in a mixture of 4g \[\ce{O2}\] and 2g \[\ce{H2}\] confined in a total volume of one litre at 0°C is ______.
[Given R = 0.082 L atm mol−1K−1, T = 273 K]



